1@khyati the_myth na bola naa ki Cl3- will use its 3d orbital? how? if chlorine has to uce its 3d orbital as myth told thn it has to first enter 4s orbital......im a lil unclear? Khyati plzz clear? and myth also :)
6 Answers
1if you draw the lewis structure for I3-, you'll see that the central iodine atom does not obey the octect rule. It has 5 electron domains (10 electrons). This means that its d orbitals are participating in its bonding. Fluroine is only in the second period and since there are no "2d" orbitals, it cannot form the F3- ion.
If we use this same logic than both Cl3- and Br3- should exist because the central atoms in those ions would utilize their 3d and 4d orbitals, respectively.
but Cl3- does not exist.This is probably similar to F3- in regards to the size of the atom. chlorine atom is too small for Cl3- to exist
11Well, though Br3- ion is less stable and less common than I3-
A few unstable Cl3- compounds are known, and the ion is formed in concentrated solution. This means Cl3- exist.
No F3- compounds are known
@ Shubham, Chlorine is in 3rd period usme 4th shell kyun dal rahe ho.
111Well, actually when these kinds of situation arises, the atoms directly use their 3d subshells
without using 4s. (Its a guess, but I think this is what exactly happens), that 3d
and 4s we have to take in sequence when we do electronic configuration, but here I think
electrons have enough energy to jump and get into 3d orbitals for the formation of
molecules.
71Well I think 4s --> then 3d from inside out.
But when electrons comes from outside or any other atom then 3d-->4s (Outside In) orbitals are filled up..